What is the pH of a solution with a [H+] of 1.0 x 10-4 M?

Plz answer for brainliest trolls will get deleted

Roman55 [17]

Answer:

A; C6H12O6 + 6O2

Explanation:

You can easily differentiate between the reactants and the products, as the reactants are on the left, while the products are on the right.

3 0

3 years ago

Convert 7.50 grams of glucose C6H12O6 to moles

Lera25 [3.4K]

Answer:

The number of mole is 0.04167mole

Explanation:

To convert gram to mole, we need to calculate the molecular weight of the compound

C6H12O6

C - 12

H - 1

O - 16

Molecular weight = 6 * 12 + 1 *12 + 6 * 16

= 72 + 12 + 96

= 180g/mol

To covert gram to mole

Therefore,

= 7.50g/ 180g/mol

= 0.04167 mole of glucose

3 0

3 years ago

The equilibrium constant for the reaction AgBr(s) Picture Ag+(aq) + Br− (aq) is the solubility product constant, Ksp = 7.7 × 10−

barxatty [35]

Answer:

The reaction will be non spontaneous at these concentrations.

Explanation:

$AgBr(s)\rightarrow Ag^+(aq) + Br^- (aq)$

Expression for an equilibrium constant $K_c$ :

$K_c=\frac{[Ag^+][Br^-]}{[AgCl]}=\frac{[Ag^+][Br^-]}{1}=[Ag^+][Br^-]$

Solubility product of the reaction:

$K_{sp}=[Ag^+][Br^-]=K_c=7.7\times 10^{-13}$

Reaction between Gibb's free energy and equilibrium constant if given as:

$\Delta G^o=-2.303\times R\times T\times \log K_c$

$\Delta G^o=-2.303\times R\times T\times \log K_{sp}$

$\Delta G^o=-2.303\times 8.314 J/K mol\times 298 K\times \log[7.7\times 10^{-13}]$

$\Delta G^o=69,117.84 J/mol=69.117 kJ/mol$

Gibb's free energy when concentration $[Ag^+] = 1.0\times 10^{-2} M$ and $[Br^-] = 1.0\times 10^{-3} M$

Reaction quotient of an equilibrium = Q

$Q=[Ag^+][Br^-]=1.0\times 10^{-2} M\times 1.0\times 10^{-3} M=1.0\times 10^{-5}$

$\Delta G=\Delta G^o+(2.303\times R\times T\times \log Q)$

$\Delta G=69.117 kJ/mol+(2.303\times 8.314 Joule/mol K\times 298 K\times \log[1.0\times 10^{-5}])$

$\Delta G=40.588 kJ/mol$

For reaction to spontaneous reaction: $\Delta G$ .
For reaction to non spontaneous reaction: $\Delta G>0$ .

Since ,the value of Gibbs free energy is greater than zero which means reaction will be non spontaneous at these concentrations

5 0

3 years ago

As the movement of molecules within a substance increases, describe the change in heat of the substance. Justify your response i

Vladimir [108]

It will get hotter, because the molecules create heat when they move around just like us when we run.

3 0

3 years ago

Read 2 more answers

Use LeChâtelier's principle explain why the concentration of NO at equilibrium increases when the reacuon takes place at higher

Tatiana [17]

increasing the temperature shifts the equilibrium in the direction of the reaction in which heat is absorbed.

Explanation:

The concentration of NO at equilibrium will increase when the reaction takes place at a higher temperature because increasing the temperature shifts the equilibrium in the direction of the reaction in which heat is absorbed.

The reaction is an endothermic reaction.

N₂ + O₂ + heat ⇄ 2NO

According to Le Chatelier's principle, "if any of the conditions of a system in equilibrium is changed the system will adjust itself in order to annul the effect of the change".

In an endothermic reaction, heat is usually absorbed.
We see that in the backward reaction, heat is absorbed.
If the temperature of this reaction is increased, the backward reaction is favored more.
Since the reactants are combining better, more products NO results.

learn more:

Thermodynamics of reactions brainly.com/question/10567109

#learnwithBrainly

6 0

3 years ago